1. Aluminum metal reacts with aqueous sulfuric acid to produce aqueous aluminum sulfate and hydrogen gas. If 11.3 g of aluminum reacts with 50.5 g of sulfuric acid, what is the maximum amount of aluminum sulfate that can be produced?

If 2.000 g tungsten is reacted with 0.092 mL of 12.5 M sodium hydroxide and 0.092 mL of water, how many moles of gas could be produced?

For the reaction Ca(s)+Cl2(g)→CaCl2(s) calculate how many grams of the product form when 21.4 gg of Ca completely reacts. Assume that there is more than enough of the other reactant.

The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.

A student knows the mass of one of the reactants of a chemical reaction and wants to calculate the mass of one of the products of the reaction. Which process should the student follow? Multiply the mass of the reactant by its molar mass to find the number of moles of the reactant. Use the chemical equation to find the number of moles of the product. Multiply the number of moles of the product by its molar mass to find the mass of the product. Multiply the mass of the reactant by its molar mass to find the number of moles of the reactant. Use the chemical equation to find the number of moles of the product. Divide the number of moles of the product by its molar mass to find the mass of the product. Divide the mass of the reactant by its molar mass to find the number of moles of the reactant. Use the chemical equation to find the number of moles of the product. Multiply the number of moles of the product by its molar mass to find the mass of the product. Divide the mass of the reactant…

For the reaction Ti(s) + 2 F2 (g) → TIF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants.

Consider the following data gathered in the "Molar Mass of a Gas" experiment.   * Mass of the empty reaction test tube: _____27.54_____ g * Mass of the test tube and MnO2 used in the reaction: ____28.04___ g * Mass of the test tube, KClO3 (MM = 122.55 g/mol) and MnO2 used in the reaction: ____29.31___ g * Mass of the test tube and its contents after the reaction: ____ (2.87x10^1) _____ g * Volume of the bubble of oxygen generated in the experiment: ___356___ mL * Atmospheric pressure in the lab: ______766.06______ mm Hg * Vapor pressure at reaction temperature: _____18.6_____ m Hg   Calculate the mass of oxygen generated in the reaction

Aqueous sulfuric acid (H,SO,) will react with sold sodium hydroxide (NaH) to produce aqueous sodium sulfate (Na,SOp) and liquid water (H,O). Suppose 51.0 g of sulfuric acid is mixed with 80. g of sodium hydroxide. Calculate the maximum mass of sodium sulfate that could be produced by the chemical reaction.

A materials scientist has created an alloy containing aluminum, copper, and zinc, and wants to determine the percent composition of the alloy. The scientist takes a 12.849 g sample of the alloy and reacts it with concentrated HCl. The reaction converts all of the aluminum and zinc in the alloy to aluminum chloride and zinc chloride in addition to producing hydrogen gas. The copper does not react with the HCl. Upon completion of the reaction, a total of 10.4 L of hydrogen gas was collected at a pressure of 724 torr and a temperature of 27.0 °C. Additionally, 2.836 g of unreacted copper is recovered. Calculate the mass of hydrogen gas formed from the reaction. mass: ----- g Calculate the mass of aluminum in the alloy sample. mass: ---- g What is the mass percent composition of the alloy? Cu: -----% Zn: ----% Al: -----%

For the following reaction, 4.77 grams of hydrogen gas are allowed to react with 48.5 grams of iodine. hydrogen (g) + iodine (s) hydrogen iodide (g) What is the maximum amount of hydrogen iodide that can be formed? grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? grams